Chemistry & Chemical Reactivity
9th Edition
ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 12, Problem 11PS
Predict the trend in lattice energy, from least negative to most negative, for the following compounds based on the ion charges and ionic radii; LiI, LiF, CaO, RbI.
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The lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na–F
distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: 682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol, or 3175 kJ/mol? Explain your answer.
Which substance do you expect to have the greatest lattice energy: MgF2, CaF2, or ZrO2? Why?
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The lattice energy of LiF is 1023 kJ/mol, and the Li–F distance is 200.8 pm. NaF crystallizes in the same structure as LiF but with a Na–F distance of 231 pm. Which of the following values most closely approximates the lattice energy of NaF: 510, 890, 1023, 1175, or 4090 kJ/mol? Explain your choice.
Chapter 12 Solutions
Chemistry & Chemical Reactivity
Ch. 12.1 - (a) Determining an Atom Radius from Lattice...Ch. 12.1 - Prob. 1RCCh. 12.1 - Prob. 2RCCh. 12.2 - If an ionic solid has an fcc lattice of anions (X)...Ch. 12.2 - Potassium chloride has the same unit cell as NaCl....Ch. 12.2 - 1. The unit cell of silicon carbide. SiC is...Ch. 12.2 - If one edge of the silicon carbide unit cell is...Ch. 12.2 - Prob. 1QCh. 12.2 - Describe the unit cell of lithium (see Figure).Ch. 12.2 - Prob. 3Q
Ch. 12.2 - Prob. 4QCh. 12.3 - Prob. 1RCCh. 12.3 - Prob. 2RCCh. 12.3 - Prob. 3RCCh. 12.4 - Prob. 1RCCh. 12.5 - Prob. 1QCh. 12.5 - Prob. 2QCh. 12.5 - Prob. 3QCh. 12.5 - 1. Which of the following allotropes of carbon is...Ch. 12.5 - Prob. 2RCCh. 12.6 - Prob. 1RCCh. 12.6 - Suppose you wanted to cool 100. g of water from 20...Ch. 12.7 - Prob. 1RCCh. 12.7 - How many tin atoms are contained in the tetragonal...Ch. 12.7 - Prob. 2QCh. 12.7 - Prob. 3QCh. 12.7 - Prob. 4QCh. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Outline a two-dimensional unit cell for the...Ch. 12 - Prob. 3PSCh. 12 - Rutile, TiO2, crystallizes in a structure...Ch. 12 - Cuprite is a semiconductor. Oxide ions are at the...Ch. 12 - The mineral fluorite, which is composed of calcium...Ch. 12 - Calcium metal crystallizes in a face-centered...Ch. 12 - The density of copper metal is 8.95 g/cm3. If the...Ch. 12 - Potassium iodide has a face-centered cubic unit...Ch. 12 - A unit cell of cesium chloride is illustrated in...Ch. 12 - Predict the trend in lattice energy, from least...Ch. 12 - Prob. 12PSCh. 12 - To melt an ionic solid, energy must be supplied to...Ch. 12 - Which compound in each of the following pairs...Ch. 12 - Prob. 15PSCh. 12 - Prob. 16PSCh. 12 - Considering only the molecular orbitals formed by...Ch. 12 - Prob. 18PSCh. 12 - Prob. 19PSCh. 12 - Prob. 20PSCh. 12 - Prob. 21PSCh. 12 - Prob. 22PSCh. 12 - Prob. 23PSCh. 12 - Prob. 24PSCh. 12 - A diamond unit cell is shown here. Unit cell of...Ch. 12 - The structure of graphite is given in Figure...Ch. 12 - We have identified six types of solids (metallic,...Ch. 12 - Prob. 28PSCh. 12 - Classify each of the following materials as...Ch. 12 - Prob. 30PSCh. 12 - Benzene, C6H6, is an organic liquid that freezes...Ch. 12 - The specific heat capacity of silver is 0.235 J/g ...Ch. 12 - Prob. 33PSCh. 12 - Prob. 34PSCh. 12 - Prob. 35PSCh. 12 - If your air conditioner is more than several years...Ch. 12 - Sketch a phase diagram for O2 from the following...Ch. 12 - Tungsten crystallizes in the unit cell shown here....Ch. 12 - Silver crystallizes in a face-centered cubic unit...Ch. 12 - The unit cell shown here is for calcium carbide....Ch. 12 - The very dense metal iridium has a face-centered...Ch. 12 - Vanadium metal has a density of 6.11 g/cm3....Ch. 12 - Prob. 43GQCh. 12 - Prob. 44GQCh. 12 - Prob. 45GQCh. 12 - Consider the three types of cubic units cells. (a)...Ch. 12 - The solid-state structure of silicon is shown...Ch. 12 - The solid-state structure of silicon carbide is...Ch. 12 - Spinels are solids with the general formula AB2O4...Ch. 12 - Using the thermochemical data below and an...Ch. 12 - Prob. 51GQCh. 12 - Prob. 52GQCh. 12 - Prob. 53GQCh. 12 - Prob. 54GQCh. 12 - Prob. 55GQCh. 12 - Prob. 56GQCh. 12 - Like ZnS, lead(II) sulfide, PbS (commonly called...Ch. 12 - CaTiO3, a perovskite, has the structure below. (a)...Ch. 12 - Potassium bromide has the same lattice structure...Ch. 12 - Calculate the lattice energy of CaCl2 using a...Ch. 12 - Why is it not possible for a salt with the formula...Ch. 12 - Prob. 63SCQCh. 12 - Prob. 64SCQCh. 12 - Prob. 65SCQCh. 12 - Phase diagrams for materials that have allotropes...
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- 7.74 In a lattice, a positive ion is often surrounded by eight negative ions. We might reason, therefore, that the lattice energy should be related to eight times the potential of interaction between these oppositely charged particles. Why is this reasoning too simpler?arrow_forwardThe lattice energy of KF is 794 kJ/mol, and the interionic distance is 269 pm. The Na—F distance in NaF, which has the same structure as KF, is 231 pm. Which of the following values is the closest approximation of the lattice energy of NaF: 682 kJ/mol, 794 kJ/mol, 924 kJ/mol, 1588 kJ/mol, or 3175 kJ/mol? Explain your answer.arrow_forwardWrite all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forward
- Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.arrow_forwardExplain the decomposition of nitroglycerin in terms of relative bond enthalpies.arrow_forwardWhat main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.arrow_forward
- Compare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?arrow_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forwardWhich statement(s) is/are true about bond enthalpy? (a) The bond energy for a triple bond between A and B is three times that of a single bond between A and B. (b) H for the breaking of a bond is always a negative number. (c) Energy is required to make a bond. (d) Bond enthalpy is defined only for bonds broken or formed in the gaseous state. (e) The presence of bonds does not influence the geometry of a molecule. However, the presence of bonds affects the value of the bond enthalpy between two atoms.arrow_forward
- The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?arrow_forwardThe lattice energy of LiF is 1023 kJ/mol, and the LiF distance is 201 pm. MgO crystallizes in the same structure as LiF but with a Mg—O distance of 205 pm. Which of the following values most closely approximates the lattice energy of MgO: 256 kJ/mol, 512 kJ/mol, 1023 kJ/mol, 2046 kJ/mol, or 4008 kJ/mol? Explain your choice.arrow_forwardDraw resonance structures for each of these ions: NSO− and SNO−. (The atoms are bonded in the order given in each case, that is, S is the central atom in NSO−.) Use formal charges to determine which ion is likely to be more stable. Explain why the two ions cannot be considered resonance structures of each other.arrow_forward
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